2 AgBr(aq) +2 Hg(l)2 Ag(s) + Hg2Br2(s) given the following standard reduction potentials. Hg2Br2(s) + 2 e 2 Hg(l) + 2 Br (aq) E° = +0.140 %3D E° = +0.071 AgBr(aq) + e - Ag(s) + Br (aq) %3D O a. +0.069 V Ob.-0.069 V

Q: Calculate the Eºcell and AGo for the reaction 2Br (aq) + F₂(g) → Br₂(1) + 2F-(aq) Given the…

A: Answer. Spontaneous reaction is one in which the value of Gibbs free energy is negative.

Q: Given the following standard reduction potentials: Fe³+ (aq) + e Fe²+(aq), E°= +0.77V - O₂(g)+ 4 H…

A: The electrode which is having a higher reduction potential gets reduced at the cathode while the…

Q: Consider the standard reduction potentials listed below and identify the substance that will act as…

A: For checking strongest oxidising agent we first of all check which species have highest reduction…

Q: half-reaction standard reduction potential 2+ Zn (aq)+2e Zn(s) E=-0.763 V red HNO,(aq)+H (aq)+e…

A: Using concept of galvanic cell we can solve this problem. From given half cell data.

Q: Given the following 2AgCl(s) +X(s) → 2Ag(s) + 2Cl-(aq) + X2+(aq)         E°cell = 0.73 V and…

A: Given reaction: 2AgCl(s) +X(s) → 2Ag(s) + 2Cl-(aq) + X2+(aq)         E°cell = 0.73 V AgCl(s) → Ag(s)…

Q: 31. Calculate AG° for the following galvanic cell: Mn(s) | Mn²"(aq) || Fe"(aq) [Fe(s), given these…

A:

Q: Consider the standard reduction potentials and redox couples used in a galvanic cell. Unbalanced…

A:

Q: Calculate the maximum amount of work produced by the cell when the partial pressure of O₂ is 0.2050…

A:

Q: Use standard reduction potentials to calculate the standard free energy change in kJ for the…

A:

Q: Use the standard reduction potentials below to determine which element or ion is the best reducing…

A: Answer:The specie that reduces others and itself gets oxidized during the redox reaction is called…

Q: Select the pair of products formed in the electrolysis of a solution of ZrCl4(aq) using inert…

A: The objective of the question is to find the pair of products formed in the electrolysis of a…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.867 M…

A: Given- Cr(s)+Sn2+(aq) <->Cr2+(aq)+Sn(s) [Cr2+]=0.867M  [Sn2+]=0.0110M

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: A redox reaction is an electron transfer process where oxidation and reduction reactions occur…

Q: If the voltmeter was replaced with a resistor (that allows current to flow) and the current is…

A:

Q: at 25 ° C, the galvanic element Pt | MnO4- 0.1M, Mn2 + 0.1M, pH = 1 || Ag + 0.0001M | Ag has the…

A: Welcome to bartleby !

Q: Using the following standard reduction potentials, Fe3+(aq) + e- → Fe2+(aq) E° = +0.77 V Cu2+(aq) +…

A: The standard cell potential (Eocell) for the cell is determined  using the following equation…

Q: Consider the battery represented by the following notation. Ni(s) | Ni*"(aq) || Ag*(aq) | Ag(s)…

A:

Q: Met (aq)+N(s) - N+ (aq) + M(s)' The standard reduction potentials are: M+ (aq) + ae M(s) e =0.400 V…

A: The given half reactions are The Nernst equation for (1) is The Nernst equation for (2) is For…

Q: What is E°(cell) for the cell Mn | Mn²⁺(aq) || Ag⁺(aq) | Ag?   Standard Reduction Potential: Au³⁺(aq…

A: Thank you.

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A:

Q: When an aqueous solution of potassium iodide is electrolyzed using platinum electrodes, the…

A: 8.15mA current flows which is equal to 0.00815A time is 12.6min = 756s The molar mass of I2 =…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: Relation between standard cell potential and standard Gibbs free energy change is shown below:…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2 +] = 0.887 M…

A:

Q: The standard cell potential for the reaction at 298.15 K: Fe (s) + Zn2+ (aq) ⇋ Fe2+ (aq) + Zn (s)…

A:

Q: Standard Reduction Potentials (Volts) at 25 °C Cl2 (g) + 2 e-  2 Cl- (aq) 1.360 O2(g) + 4 H3O+(aq) +…

A: The process of electrolysis is a combination of oxidation and reduction. When any element releases…

Q: All of our standard reduction potentials are supposed to be at "standard acidic conditions, which…

A:

Q: Calculate the cell potential given the standard reduction potentials for the half-reactions of the…

A:

Q: The following half reactions are used for a galvanic cell: Zn2+(aq)+2e-→Zn(s)E°=-0.76V…

A: Nerst Equation:Where,E is the cell potential under non-standard conditions.E∘ is the standard cell…

Q: Calculate the Kf of Ag(NH₃)₂ from Ag⁺(aq) +e⁻⇌Ag(s) E°=0.80 V ;Ag(NH₃)₂⁺(aq)+ e⁻⇌Ag(s)…

A: The given reactions along with their reduction potential values are, Ag+aq+e-↔Ags    E°=0.80…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: Answer: Relation between standard cell potential and standard Gibbs free energy change is shown…

Q: E°(V). -1.66 3+ + 3e¯→ Al(s) +0.07 gBr(s) + e¯→ Ag(s) + Br¯ 4+ + 2e → Sn 2+ +0.14 ° 3+ + e¯→ Fe2+…

A: Loss of electrons is oxidation.  Gain of electron is reduction. Species undergo oxidation is…

Q: Use the following standard reduction potentials to determine which species is the strongest reducing…

A: ->The species which has highest reduction potential that will get reduce itself and oxidize…

Q: Consider the following reaction and its AG AG° = -408.0 kJ/mol Mg(s) + Ni?+(aq) → Mg²+(aq) + Ni(s)…

A: Given-> Mg(s) + Ni2+(aq) ----> Mg2+(aq) + Ni(s)  ∆G° = -408.0 KJ/mole = -408000 J/mole (1 KJ =…

Q: Using the standard electrode potentials: Cl2(g) + 2e 2CI (aq) E° = +1.36 V; Cd2*(aq) + 2e- Cd(s) E°…

A: In the electrochemical cell, the chemical energy is converted into electrical energy. The addition…

Q: In the following: Al³+ (aq) + 3 e Al(s) E° = -1.66 V Cr³+ (aq) + 3e →→ Cr(s) E° = -0.74 V What is…

A:

Q: Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box…

A: We will predict the electrolysis product by using standard reduction potential values .

Q: Using standard reduction potentials, calculatethe standard emf for each of the following…

A: (a) Cl2(g) + 2 I-(aq)---->2 Cl-(aq) + I2(s) Cl2(g) → 2 Cl-   Eₒ = 1.36 , Reduction on cathode  2…

Q: sing the following standard reduction potentials: Ag+ (aq) + e- ⇌ Ag (s) E o = +0.80 V Pb2+ (aq) +…

A: Electrons flow from anode to cathode anode is negatively charged and cathode is positively charged .…

Q: Given the standard reduction potential, E°, which of the following half-reactions contain the…

A:

Q: that should be written in the spaces in the text given below in the box below. ……………………… can form…

A: Write the expressions that should be written in the spaces in the text given below in the box below.…

Q: Given the following standard reduction potentials, E°red, which species has the  greatest tendency…

A: In an electrochemical cell, the electrode with a higher standard reduction potential acts as a…

Q: Calculate the [Ni2+] in the following galvanic cell, given that the measured voltage of the cell is…

A:

Q: When an aqueous solution of potassium iodide is electrolyzed using platinum electrodes, the…

A: Given, Current flow (I) = 8.15mA = 8.15×10-3A Time = 12.6 min = 756S 2I–(aq) → I2(aq) + 2e(Anode…

Q: Which of the following substances is the strongest oxidizing agent?

A: Oxidizing agent are substances which reduces itself and oxidizes other species.

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+] = 0.875 M…

A: The given cell reaction is : Zn2+=0.875 MFe2+=0.0200 M

Q: Use standard reduction potentials to calculate the standard free energy change in kj for the…

A: We have to calculate the standard Gibbs free energy change and the equilibrium constant value.…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: Answer: Relation between standard Gibbs free energy change and standard cell potential is shown…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A:

Q: Mn(k) | Mn²+(0.2 M) || H+ (pH= ?) | H2 (g, 1.5 atm) | The cell potential of the Pt(k) Cell was found…

A:

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.